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WorksheetsBIOL 112: Principles of Biology II: TYU 2: Basic GC for Biology
Total questions: 71
Worksheet time: 36mins
Evaluate the following statement: oxygen is not a greenhouse gas; therefore, gases containing oxygen, such as carbon dioxide, are not greenhouse gases either.
True. Because oxygen is not a greenhouse gas, it is unlikely to combine with anything at a higher level of organization to form a greenhouse gas.
True. Compounds display emergent properties that are very similar to the elements that form them.
False. Compounds can have emergent properties that are very different from the elements that form them.
False. Oxygen is a special case because of its reactivity and electronegativity.
True. It is impossible for a gas containing oxygen to be a greenhouse gas.
There are ____ naturally occurring elements.
4
25
92
108
238
Which is a trace element?
nitrogen
copper
carbon
hydrogen
oxygen
What are the four most abundant elements found in living systems?
hydrogen, oxygen, calcium, and nitrogen
hydrogen, oxygen, nitrogen, and carbon
hydrogen, oxygen, nitrogen, and carbon dioxide
nitrogen, carbon, sulfur, and oxygen
magnesium, calcium, iron, and zinc
Adding proton number and neutron number, what would be the result?
electron number
neutron number
atom
atomic mass number
proton number
Which subatomic particlesis electrically neutral?
elements
protons
molecules
neutrons
electrons
The number of protons in an uncharged atom _____.
equals the number of electrons in the outer orbital of the atom
equals the number of electrons
determines its mass number
varies with the different isotopes
equals the number of neutrons
Consider a hypothetical atom with an atomic number of 4 and an atomic mass of 9.0. How many neutrons does this atom have?
one
three
four
five
None of the choices is correct.
An uncharged atom of nitrogen (atomic number = 7) has ______.
seven neutrons
seven protons and seven electrons
seven valence electrons
seven neutrons and seven electrons
seven protons and seven neutrons
Isotopes of an element will always differ in ______.
atomic number
number of electrons
number of protons
atomic mass
None of the listed responses is correct.
A particular carbon isotope has an atomic number of 6 and an atomic mass of 14. The respective number of neutrons, protons, and electrons in an electrically neutral atom if this isotope of carbon is ______.
8, 6, and 8
6, 6, and 8
8, 6, and 4
8, 6, and 6
6, 8, and 6
Phosphorus-32 (radioactive) has ______ than phosphorus-35 (normal).
three more protons
three fewer protons
three more neutrons
three more electrons
three fewer neutrons
The most common form of calcium has 20 protons, 20 neutrons, and 20 electrons. Which of the following elements would be an isotope of calcium?
an atom with 20 protons, 20 neutrons, and 18 electrons
an atom with 21 protons, 20 neutrons, and 21 electrons
an atom with 20 protons, 21 neutrons, and 20 electrons
an atom with 21 protons, 21 neutrons, and 21 electrons
All of the listed responses are correct.
Radioactive isotopes are useful in scientific research because ______.
they are not readily incorporated into biological reactions
they are difficult to detect in small amounts, but living cells cannot distinguish them from the corresponding stable isotopes
they decay spontaneously and give off energy and subatomic particles
they can be used as tracers to follow particular atoms and molecules through metabolic pathways, especially in medicine
All of the listed responses are correct.
Potassium (atomic number 19, mass number 40) and sodium (atomic number 11, mass number 23) have similar chemical properties and reactive behavior. This is because uncharged atoms of potassium and sodium _______.
have different atomic numbers but the same number of electrons
have different atomic numbers, different mass numbers, and different numbers of electrons in their outermost electron shells
have different mass numbers and each has one electron in its outermost electron shell
have different atomic numbers and different numbers of electrons in their outermost electron shells
have the same atomic number and each has one electron in its outermost electron shell
The chemical characteristics or reactivity of an element depend mostly on the _______.
mean energy level of its electrons
number of electron shells present in the atoms
degree to which it has more or fewer electrons than protons
number of protons plus the number of neutrons
number of electrons in its outermost shell
Some groups of elements react chemically in similar ways. For example, the chemistry of sodium and the chemistry of lithium are similar. The chemistry of chlorine and the chemistry of iodine are also similar. These similarities in chemistry result when different elements have similar _______.
total numbers of electrons
atomic size
energy quanta per electron
atomic numbers
numbers of outer-shell electrons
How many electrons would be present in the valence shell of a sulfur atom (atomic number 16, mass number 32)?1
one electron
eight electrons
four electrons
six electrons
two electrons
For most atoms, a stable configuration of electrons is attained when the atom ______.
has as many protons as neutrons
has a full number electrons in its outermost shell
has moved all its electrons to its outermost shell
achieves a zero net charge
None of the choices is correct.
An atom that normally has _____ in its outer shell would not tend to form chemical bonds with other atoms.
one electron
three electrons
four electrons
six electrons
eight electrons
When one or more pairs of valence electrons are shared by two neutral atoms, what type of bond is formed?
a covalent bond
a hydrogen bond
an electronegative bond
a van der Waals bond
an ionic bond
A polar covalent bond is a bond that ______.
shares electrons equally between atoms
is found only in molecules containing oxygen
the electrons of the bond are not shared equally
is found only in H2O
ionizes
A covalent bond is likely to be polar if ______.
one of the atoms sharing electrons is much more electronegative
the two atoms sharing electrons are of the same element
it is between two atoms that are both very strong electron donors
the two atoms sharing electrons are equally electronegative
it is between two atoms that are both very strong electron acceptors
When two atoms are so unequal in their attraction for valence electrons that the more electronegative atom strips an electron completely away from its partner, the two resulting oppositely charged atoms (or molecules)_______.
form a covalent bond with another atom
are ions
gain or lose a neutron
gain or lose a proton
become part of a molecule
A sodium atom has a mass number of 23. Its atomic number is 11. How many electrons does it have if it is not an ion?
11
12
22
23
34
Copper has an atomic number of 29 and a mass number of 64. What would result if an uncharged copper atom lost two electrons?
The atomic number of the atom would remain 29, the mass number would be reduced to 62, and the atom would be an anion.
The atomic number would be reduced to 27, the mass number would remain 64, and the atom would be an anion with a +2 charge.
The atomic number would remain 29, the mass number would remain 64, and the atom would be a cation with a +2 charge.
The atomic number would remain 29, the mass number would increase to 66, and the atom would be a cation with a −2 charge.
The atom would have a double-negative charge and be an ion.
The compound CaSO4 ionizes into a calcium ion and a sulfate ion (SO4). Calcium has two electrons in its outer shell. Upon ionization, what would you expect the charge on the sulfate ion to be?
−4
−2
−1
+1
+2
Ionic bonds form as a result of ______.
attraction between ions that have opposite charges
the asymmetric distribution of electrons in constant motion
attraction between hydrogen and other atoms that share electrons unequally
sharing of electron pairs between atoms
unequal sharing of electrons between atoms
A hydrogen bond ______.
is a weak chemical bond
is one in which hydrogen is strongly attracted to a positively charged atom
is one in which two hydrogen atoms bond to each other
is a strong chemical bond
is a function of hydrophobic interactions
What is the role of van der Waals interactions in biological molecules?
Van der Waals interactions are too weak to be significant.
Van der Waals interactions are strong bonds that play a major structural role in holding proteins together.
Although they are weak bonds, van der Waals interactions involve the sharing of electrons.
Van der Waals interactions are only important in water.
Although they are weak bonds, van der Waals interactions help to reinforce the three-dimensional shapes of large molecules and help hold membranes together.
Which molecule has the shape of a completed tetrahedron?
glucose (C6H12O6)
hydrogen gas (H2)
methane (CH4)
oxygen gas (O2)
water (H2O)
Pharmaceutical researchers are often interested in blocking particular receptor proteins on cell surfaces. What chemical property of a molecule would be most important for this?
the number of valence electrons
the molecule's shape
the type of bonding in the molecule
the number of double bonds in the molecule
the atomic numbers of the atoms involved
Which of the following statements is true about chemical reactions?
They represent the way matter is created and destroyed.
Only inorganic molecules can participate in chemical reactions.
They reach chemical equilibrium when the amounts of products and reactants are equal.
They may have different numbers of a given atom on each side of the equation arrow.
They involve the making and breaking of chemical bonds, leading to changes in the composition of matter.
Which statement describes a reversible reaction that has reached chemical equilibrium?
The concentration of the reactants is equal to the concentration of the products.
The forward and the reverse reactions have stopped.
The rate of the forward reaction exceeds the rate of the reverse reaction.
The rate of the reverse reaction equals the rate of the forward reaction.
The rate of the reverse reaction exceeds the rate of the forward reaction.
Cells are surrounded by water, and cells themselves consist of about 70–95% water. Which choice best describes an emergent property of living things which derives from this fact?
A variety of nutrient molecules is readily available as dissolved solutes.
The temperature of living things tends to change relatively slowly.
Dissolved substances can be easily transported within a cell or between cells in multicellular organisms.
Waste products produced by cell metabolism can be easily removed.
All of the listed responses are correct.
Water is a polar molecule. This means that ______.
the opposite ends of the molecule have opposite electrical charges
water molecules are linear, like a pole
the atoms in water have equal electronegativities
water is one of the many hydrophobic molecules
All of the listed responses are correct.
The partial charges on a water molecule occur because of ____.
the high electronegativity of hydrogen
covalent bonding
the unequal sharing of electrons between the hydrogen and the oxygen atoms of a water molecule
the achievement of a stable configuration by one atom of a bond but not by the other partner
widespread ionization
In a group of water molecules, hydrogen bonds form between ______.
the hydrogen atoms in a single water molecule
the oxygen atom in one water molecule and a hydrogen atom in another water molecule
two hydrogen atoms in different water molecules
the oxygen atoms in different water molecules
None choices is correct.
If water were not a polar molecule, how would the effects of warming climate be different?
The effects would be drastically worse because the loss of the polar nature of water would greatly reduce its specific heat and its ability to moderate temperature.
The effects would be worse because a loss of the polar molecular structure would lead to a greater amount of heat absorbed by water molecules and, thus, an increase in its specific heat.
The effects would be only slightly worse because there are other polar molecules, such as methane, with only slightly lower specific heat values than water that can moderate climate as water does.
The effects would be marginally different due to the fact that water, as a polar molecule, is a greenhouse gas in its vapor state.
None of the choices accurately describes how and why the effects would differ.
The tendency of water molecules to stay close to each other as a result of hydrogen bonding _____.
keeps water moving through the vessels in a tree trunk
provides the surface tension that allows leaves to float on water
is called cohesion
acts to moderate temperature
All of the choices are correct.
What do cohesion, surface tension, and adhesion have in common with reference to water?
All are produced by covalent bonding.
All are results of the structure of the hydrogen atom.
All are aspects of a crystalline structure.
All are properties related to hydrogen bonding.
All have to do with ionic interactions.
Most of water's unique features (for example, its versatility as a solvent, ability to moderate temperature, and cohesive behavior) result from the fact that _____.
hydrogen is the only element without any neutrons
oxygen has only one stable isotope, but hydrogen has three
oxygen attracts electrons more than hydrogen does
oxygen has two unfilled electron shells
More than one of the above is correct.
The ability of water molecules to form hydrogen bonds with other water molecules and water's ability to dissolve substances that have charges or partial charges are ______.
both caused by water's ability to form covalent bonds with hydrophobic substances
both caused by water's partial charges
due to water's partial charges and low molecular mass, respectively
both caused by water's two electron shells
both due to water's low molecular mass
Adhesion is best described as ______.
the process by which a crystalline lattice forms
a property of water that helps moderate Earth's temperature
the clinging of one substance to another substance
the process that contributes to the transport of water and dissolved nutrients in plants by causing water molecules to tug on other water molecules
None of the choices is correct.
You can fill a glass of water to just slightly above the rim without it spilling over the glass. What property of water allows this?
evaporative cooling
polarity
surface tension
adhesion
None of the choices is correct.
Which action would involve the greatest transfer of heat?
cooling 10 g of water from 80°C to 40°C
changing the temperature of 1 g of water from 10°C to 90°C
condensing 5 g of steam to liquid water
evaporating 1 g of water at 25°C
raising the temperature of 10 g of ethyl alcohol by 25°C
Imagine that organisms consisted of 70–95% alcohol instead of 70–95% water. Alcohol's specific heat is about half that of water. How would living things be different?
Organisms would be able to live in a much wider range of temperatures.
Living organisms would have to be much smaller.
Systems for temperature regulation would have to be much more efficient.
Warm-blooded organisms would require less insulation, such as fur or feathers.
None of the choices is correct.
The amount of heat required to change the temperature of 1 g of any substance by 1°C is defined as ______.
1 kilocalorie
the heat of vaporization of that substance
1 calorie
the specific heat of that substance
molecular cohesion
The amount of heat required to convert 1 g of any substance from the liquid to the gaseous state is defined as _____.
molecular cohesion
1 calorie
the heat of fusion of that substance
the specific heat of that substance
the heat of vaporization of that substance
The reason that coastal climates are more moderate than inland climates is due primarily to water's high _______.
surface tension
heat of fusion
density
heat of vaporization
specific heat
Sweating has a cooling effect because of water's high ______.
buffering capacity
Density
surface tension
specific heat
heat of vaporization
Because molecules of water are farther apart in ice than in liquid water, ______.
ice is denser than liquid water
ice vaporizes before liquid water does
ice expands when it melts
ice floats on liquid water
All of the choices are correct.
Water is a very versatile solvent because water molecules are ______.
volatile
nonpolar
polar
ionic
hydrophobic
How does the polarity of water contribute to its ability to dissolve so many substances?
Natural water has a pH of approximately 5.6, which is slightly acidic. Acids can dissolve more substances than bases.
Because it is polar, water forms ionic bonds with the ions in substances such as NaCl (salt).
Water's polarity allows it to form covalent bonds with many substances.
Because it is polar, water is able to interact with and dissolve hydrophobic substances.
Because it is polar, water's oppositely charged ends are attracted to positively and negatively charged ions and molecules. Water molecules form a hydration shell around oppositely charged particles.
Nonpolar molecules that cluster away from water molecules are called ______ molecules.
hydrophobic
hydrophilic
ionic
covalent
None of the choies is correct.
A molecule that has all nonpolar covalent bonds would be ______.
hydrophobic
basic (alkaline)
ionic
acidic
hydrophilic
Hydrophobic molecules are _______ water.
polarized by
attracted to
unable to interact with
absorbed by
neutralized by
Why are cell membranes composed primarily of hydrophobic molecules?
Cell membranes must be composed of polar molecules in order to interact with the aqueous solutions inside of cells.
In order to perform their function of separating the aqueous solutions outside of cells from the aqueous solutions inside of cells, cell membranes cannot be soluble in water.
In order to maintain a proper pH, cell membranes must be hydrophobic.
Cell membranes must be hydrophobic in order to form colloids.
Cell membranes must be composed of nonpolar molecules in order to form a hydration shell around the cell.
Hydrophilic substances, unlike hydrophobic substances, ______.
give up electrons to solvents
accept electrons from solvents
are repelled by water
have charges and/or partial charges to which water molecules can adhere
have a higher bond energy than water
Some substances, such as oil and gasoline, will not dissolve in water because _______.
they do not ionize
oil and gasoline are organic compounds
their electrons are so stable that they do not exchange atoms with water molecules
their molecules are so large
their molecules have no charges or partial charges to which water molecules can adhere
A mole of ethyl alcohol weighs 46 g. How many grams of ethyl alcohol are needed to produce 1 L of a 2-millimolar (2 mM; 0.002 moles per L) solution?
92 g
9.2 g
0.92 g
0.092 g
0.0092 g
An acid is ______.
a compound that donates hydrogen ions to a solution
any compound that accepts hydrogen ions
a material that resists changes in the pH of a solution
any compound with a pH
a solution with a pH between 7 and 14
Adding acid tends to ______ of a solution.
decrease the hydrogen ion concentration and lower the pH
increase the hydrogen ion concentration and raise the pH
either increase or decrease the pH, depending on the original acidity
decrease the hydrogen ion concentration and raise the pH
increase the hydrogen ion concentration and lower the pH
Which describes the dissociation of an acid?
NH3+ H+ → NH4+
KOH → K++ OH−
HF → H+ + F−
H2O → H+ + OH−
NaOH → Na+ + OH−
A glass of grapefruit juice, at pH 3, contains _______ H+ as a glass of tomato juice, at pH 4.
one-tenth as much
half as much
twice as much
three times as much
ten times as much
A solution at pH 6 contains ____ than the same amount of solution at pH 8.
100 times more H+
4 times more H+
2 times more H+
4 times less H+
100 times less H+
Adding a base tends to _____ of a solution.
lower the hydrogen ion concentration and increase the pH
lower the hydrogen ion concentration and lower the pH
increase the hydrogen ion concentration and lower the pH
lower the hydroxide ion concentration and lower the pH
increase the hydrogen ion concentration and increase the pH
When the pH of a solution shifts from 7 to 3, how has the hydrogen ion concentration changed?
It has not changed.
It has increased by 10,000 times.
It has decreased by 4 times.
It has decreased by 10,000 times.
It has increased by 4 times.
A substance that minimizes changes in the concentration of H+ and OH in a solution is a _______.
buffer
strong acid
strong base
hydrocarbon
NaCl
Sucrose has a molecular mass of 342 daltons. To make a 2 molar (2 M; 2 moles per L) solution of sucrose, _____.
stir 684 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 2 L
stir 342 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 2 L
stir 342 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 0.5 L
stir 684 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 0.5 L
stir 342 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution to 1 L
Why would more carbon dioxide taken up by the oceans cause concern?
The buffering action of carbonic acid (H2CO3) causes the pH of seawater to rise.
More carbon dioxide causes an increase in carbonic acid (H2CO3), which leads to a decrease in the concentration of carbonate ion (CO32−).
There is no cause for concern. Carbonic acid (H2CO3) is an excellent buffer and will help keep the pH of seawater constant.
More carbon dioxide causes an increase in carbonic acid (H2CO3), which leads to an increase in the concentration of carbonate ion (CO32−).
None of the choices is correct.
